Download LaBrake, Fundamentals Diagnostic Questions

LaBrake, Fundamentals Diagnostic Questions:
These are questions to be used to help you fully prepare for 1A. While these topics will be covered in the
1ABC series, they will only be covered extremely briefly. It is expected that your chemistry background
has prepared you to handle questions of this nature. Various sources can be used to help you learn the
material here if you aren’t able to complete the problems. The Atkins, “Chemical Principles” book,
which is required for the general chemistry series, covers these topics in the “Fundamentals” section if
you would like a text book for reference.
1. Assuming the following numbers are measurements and using the rules for significant figures, determine the
answer for the following calculation.
(2 x 2.4) + (361 /1.7) + (3.5 × 102) =
a)
b)
c)
d)
e)
567.1529
567.2
567
5.7 × 102
600
2. Assuming the following numbers are measurements and using the rules for significant figures, determine the
answer for the following calculation.
(15.5/42) × 219.5 =
a)
b)
c)
d)
e)
81.0059
81.006
81.01
81.0
81
3. Assuming the following numbers are measurements and using the rules for significant figures, determine the
answer for the following equation.
10054.67 + 454.2 + 64.78 + 2891 =
a) 10862.75
b) 10862.8
c) 10863
d) 10860
e) 10900
4. How many significant figures are in the following measurements?
1 × 102 cm, 1.01 × 102 cm, 1.001 × 102 cm, 1.0010 × 102 cm, 1.00 × 102 cm, 1.00010 × 102 cm
a) 3, 3, 4, 4, 3, 5
b) 3, 3, 2, 4, 3, 5
c) 3, 3, 4, 5, 3, 6
d) 1, 3, 4, 5, 3, 6
e) 1, 3, 4, 4, 3, 5
5. The length of 5 meters is the same as (1 in = 2.54 cm)
a) 5 feet
b) 5 yards
c) 5 liters
d) 5 × 103 mm
e) 5 × 10-3 mm
6. How many grams of potatoes are equivalent to 31.2 pounds of potatoes? (1 lb = 453.6 g)
a) 14152 g
b) 10,000 g
c) 1.42 × 104 g
d) 0.06878 g
e) 6.88 × 10-2 g
7. What is the density of a pear that occupies 32 cubic centimeters and has a mass of 42 grams?
a) 2.0 g · cm-3
b) .7619 g · cm-3
c) .76 g · cm-3
d) 1.3125 g · cm-3
e) 1.3 g · cm-3
8. A small leak in a water tower drips at a rate of 72 gallons per day. Express this rate in units of milliliters per
minute. (1 gal = 3.785 L)
a) 27.4 mL · min-1
b) 28 mL · min-1
c) 190 mL · min-1
d) 1900 mL · min-1
e) 3.2 mL · min-1
9. A small leak in a water tower drips at a rate of 72 gallons per day. The water tower holds 25 000 gallons of
water. How many days will it take to empty the tower at the given rate?
a) about one month
b) about 1 year
c) about 5 years
d) about 10 years
e) about 20 years
10. A liquid has a density of 1.8 grams per milliliter. How many grams of the liquid are in 62 milliliters of the
sample?
a) 110 g
b) 220 g
c) 34 g
d) 0.029 g
e) 0.03 g
11. Density can be measured as
a) lb · ft-3
b) lb · ft-1
c) lb · ft-2
d) ft2 · lb-1
e) ft3 · lb-1
12. A liquid has a density of 1.45 grams per milliliter. How many milliters are there in a 45.0 gram sample?
a) 65.3 mL
b) 31.0 mL
c) 3.22 × 10-2 mL
d) 70.0 mL
e) 29.0 mL
13. Express 14.3 sqaure centimeters in units of square millimeters.
a) 143 mm2
b) 0.143 mm2
c) 1.43 mm2
d) 1 430 mm2
3) 14 300 mm2
14. A star athlete threw a baseball at a velocity of 97 miles per hour. Express this velocity in units of meters
per second. (1 mi = 5280 ft; 1 in = 2.54 cm)
a) 142 m · s-1
b) 361 m · s-1
c) 2600 m · s-1
d) 86 m · s-1
e) 43 m · s-1
15. Table sugar, sucrose, is an example of
a) a heterogeneous mixture
b) a homogeneous mixture
c) a mineral
d) an element
e) a compound
16. Iced tea with lemon, ice, and sugar is an example of
a) a heterogeneous mixture
b) a homogenous mixture
c) a mineral
d) an element
e) a compound
17. All of the following are considered subatomic particles, except:
a) gamma rays
b) electrons
c) protons
d) neutrons
e) positrons
18. All of the following are statements from Dalton’s atomic hypothesis, except:
a) All the atoms of a given element are identical.
b) The atoms of different elements have different masses.
c) All atoms are composed of electrons, protons, and neutrons.
d) A compound is a specific combination of atoms of more than one element.
e) In a chemical reaction, atoms are neither created nor destroyed; they exchange partners to produce new
substances.
19. All of the following statements are true regarding the nuclear model of the atom, except:
a) The positive charge is densely found in the center of the atom, while the negatively charged electrons exist
in a diffuse cloud outside the nucleus.
b) Most of the space of an atom is empty space.
c) The nuclear model in which the positive charge is held densely in the center of the atom is no longer
accepted, because it was proposed over 100 years ago.
d) In a neutral atom, the number of protons in the nucleus is equal to the number of electrons outside the
nucleus.
e) One of the most important experiments conducted to reveal the nuclear model of the atom was to bombard a
thin metal sheet with alpha particles and show that some alpha particles were deflected directly back to the
source by the positively charged, dense nucleus.
21
20. The 10
Ne isotope has:
a) 10 protons, 21 electrons, 11 neutrons
b) 10 protons, 11 electrons, 21 neutrons
c) 10 protons, 10 electrons, 11 neutrons
d) 21 protons, 11 electrons, 10 neutrons
e) 21 protons, 10 electrons, 11 neutrons
21. The 126 C isotope has:
a) 6 protons, 12 electrons, 6 neutrons
b) 6 protons, 8 electrons, 12 neutrons
c) 6 protons, 6 electrons, 6 neutrons
d) 12 protons, 12 electrons, 6 neutrons
e) 12 protons, 6 electrons, 6 neutrons
22. Which element is in the same period as carbon?
a) fluorine
b) silicon
c) lead
d) phosphorus
e) hydrogen
23. Which element is in the same group as calcium?
a) cadmium
b) cesium
c) barium
d) scandium
e) potassium
24. Which of the following is a halogen?
a) lithium
b) hydrogen
c) helium
d) fluorine
e) lithium
25. Which of the following is a nonmetal?
a) bromine
b) lithium
c) antimony
d) vanadium
e) beryllium
26. Identify the symbols for the elements sodium, silicon, boron, calcium, and sulfur, respectively.
a) S, Si, Bo, Ca, Su
b) S, Si, Bo, Ca, Su
c) Na, S, Bo, C, Su
d) Na, Si, B, C, S
e) Na, Si, B, Ca, S
27. Which of the following would be considered a binary ionic compound?
a) HCl
b) CO2
c) CO
d) H2S
e) KCl
28. Which would be considered a binary molecular compound?
a) NaCl
b) CaCl2
c) FeCl3
d) BrCl
e) BaCl2
29. All of the following monatomic ions have the correct charge, except:
a) Sr2+
b) S2c) S2+
d) Mg2+
e) O230. The proper formula unit for the binary compound formed from calcium and fluorine is:
a) CaF
b) Ca2F
c) CaF2
d) Ca2F2
e) Ca3F2
31. All of the following names and formulas are properly matched, except:
a) rubidium chloride, RbCl
b) potassium sulfide, KS
c) magnesium hydroxide, Mg(OH)2
d) iron (III) chloride, FeCl3
e) lithium nitrate, LiNO3
32. The correct formula for bromine pentachloride is:
a) Br5Cl
b) BrCl5
c) BrCl
d) Br4Cl
e) BrCl4
33. The correct name for NH4NO2 is:
a) ammonia hydronitrogen oxide
b) ammonia nitrogen oxide
c) ammonium nitrate
d) ammonium nitrite
e) ammonium nitrous acid
34. The correct name for SO3 is:
a) sulfur oxide
b) sulfur trioxide
c) sulfurous acid
d) sulfuric acid
e) trisulfur oxide
35. The correct name for Na2O is:
a) disodium monoxide
b) disodium oxide
c) sodium oxide
d) sodium dioxide
e) disodium oxyacid
36. The correct name for KClO4 is:
a) krypton chlorine tetroxide
b) krypton oxychlorine
c) potassium chlorine tetroxide
d) potassium perchlorate
e) potassium perchlorine
37. All of the following hydrocarbons are named correctly with the common names, except:
a) CH4, carbon tetrahydride
b) C2H6, ethane
c) C4H10, butane
d) C5H12, pentane
e) C10H22, decane
38. Which of the following is NOT correctly matched?
a) silicon, Si
b) sodium, Na
c) sulfur, S
d) tin, Ti
e) antimony, Sb
39. Which of the following is NOT correctly matched?
a) boron, B
b) mercury, M
c) iodine, I
d) oxygen, O
e) potassium, K
40. Which of the following common names is not correctly matched with the formula?
a) NH3, ammonia
b) H2O, water
c) C2H2, dicarbon dihyrdide
d) C2H4, ethylene
e) N2O, nitrous oxide
41. Which has more molecules: a mole of H2O or a mole of O2?
a) a mole of H2O
b) a mole of O2
c) insufficient information to answer
d) They both have the same number of molecules.
e) The answer depends on the volume of the container.
42. How many moles of hydrogen are in 3 moles of ammonia, NH3?
a) 3 moles
b) 6 moles
c) 9 moles
d) 6.0221 × 1023 moles
e) 1.80663 × 1023 moles
43. How many atoms of hydrogen are in 3 moles of ammonia, NH3?
a) 3 atoms
b) 9 atoms
c) 6.0221 × 1023 atoms
d) 1.8066 × 1023 atoms
e) 5.4199 × 1024 atoms
44. How many moles of sodium ions are there in 2.5 moles of sodium chloride, NaCl?
a) 6.0221 × 1023 moles
b) 1.5055 × 102 moles
c) 1.0 mole
d) 2.5 moles
e) 5.0 moles
45. How many moles of glucose are there in 2.4088 × 1024 molecules of glucose?
a) 4 moles
b) 2 moles
c) 6.0221 × 1023 moles
d) 1.4506 × 1048 moles
e) insufficient information to answer
46. Calculate the molar mass of copper (II) nitrate, Cu(NO3)2.
a) 187.57 g·mol-1
b) 93.56 g·mol-1
c) 125.56 g·mol-1
d) 251.12 g·mol-1
e) 198.45 g·mol-1
47. Calculate the molar mass of ammonium sulfide, (NH4)2S.
a) 47.08 g·mol-1
b) 61.09 g·mol-1
c) 68.14 g·mol-1
d) 62.10 g·mol-1
e) 75.10 g·mol-1
48. Calculate the molar mass of glucose, C6H12O6.
a) 29.02 g·mol-1
b) 116.08 g·mol-1
c) 156.21 g·mol-1
d) 174.12 g·mol-1
e) 180.16 g·mol-1
49. Calculate the number of moles of glucose, C6H12O6, in a 512 gram sample of glucose.
a) 1.42 moles
b) 2.84 moles
c) 0.352 moles
d) 9.22 × 104 moles
e) 1.71 × 1024 moles
50. Calculate the number of molecules of glucose, C6H12O6, in a 512 gram sample of glucose.
a) 1.71 × 1024 molecules
b) 8.55 × 1023 molecules
c) 6.0221 × 1023 molecules
d) 2.84 molecules
e) 9.224 × 104 molecules
51. How many grams of glucose are in 5.9 moles of glucose?
a) 31 g
b) 3.3 × 10-2 g
c) 1.1 × 103 g
d) 2.0 × 1022 g
e) 3.3 × 102 g
52. How many formula units of sodium fluoride, NaF, are in 496 g of sodium fluoride?
a) 11.8 formula units
b) 2.08 × 104 formula units
c) 1.25 × 1028 formula units
d) 7.11 × 1024 formula units
e) 1.96 × 10-23 formula units
53. What is the mass percent of oxygen in water?
a) 88.81%
b) 66.67%
c) 33.33%
d) 11.19%
e) insufficient information to answer
54. A compound containing only nitrogen and oxygen was found to contain 2.1 grams of nitrogen and 1.2
grams of nitrogen. What is the mass percent composition of oxygen and nitrogen in this compound?
a) 2.1% N, 1.2% O
b) 75% N, 25% O
c) 25% N, 75% O
d) 64% N, 36% O
e) 36% N, 64% O
55. Calculate the mass percent composition of sodium nitrate, NaNO3.
a) 27.05% Na, 16.48% N, 56.47% O
b) 43.38% Na, 26.43% N, 30.19% O
c) 27.05% Na, 16.48% N, 30.10% O
d) 20% Na, 20% N, 60% O
e) 10% Na, 10% N, 30% O
56. The mass percent composition of a particular compound was found to be 65.45% carbon, 5.492%
hydrogen, and 29.06 % oxygen. Determine the empirical formula of this compound.
a) C7H5O3
b) CHO
c) C3H3O
d) C6H12O6
e) insufficient information to answer
57. The mass percent composition of a particular compound was found to be 26.95% sulfur, 14.43% oxygen,
and 59.61% chlorine. The molar mass of the compound was determined to be 118.96 g·mol-1. Determine the
molecular formula for this compound.
a) SOCl
b) S2OCl6
c) SOCl2
d) S2O2Cl4
e) S2O2Cl2
58. Determine the empirical formula for a pure sample of a compound that contains 6.3 grams of nitrogen and
3.6 grams of oxygen.
a) N2O6
b) N3O6
c) N6O3
d) N2O
e) NO2
59. What is the molecular formula of a compound that has an empirical formula of CH and a molecular mass of
78.53 grams per mole?
a) CH
b) C3H3
c) C6H6
d) CH4
e) C6H14
60. Identify the empirical formula of C6H4Cl2.
a) C6H4Cl2
b) C6Cl2H4
c) C12H8Cl4
d) CHCl
e) C3H2Cl
61. Which of the following is NOT true?
a) A homogeneous mixture can also be referred to as a solution.
b) Within a solution, the component in the least amount is called the solute.
c) Within a solution, the component in the least amount is called the solvent.
d) A solution in which the solute is water is called an aqueous solution.
e) Solutions can exist in the liquid phase or in the gas phase.
62. All of the following are physical techniques used to separate mixtures, except:
a) filtration
b) chromatography
c) decanting
d) combustion train
e) distillation
63. What is the molarity of a solution prepared by dissolving 238 grams of potassium bromide, KBr, in water to
make a total of 5.00 × 102 milliliters of aqueous solution?
a) 4.76 × 10-1 molar
b) 4.76 × 101 molar
c) 4.00 molar
d) 4.00 × 10-3 molar
e) 5.66 × 101 molar
64. What is the molarity of a solution prepared by dissolving 457 grams of sodium nitrate, NaNO3, in water to
make a total of 2.00 liters of aqueous solution?
a) 2.69 molar
b) 9.30 × 10-2 molar
c) 1.08 × 102 molar
d) 2.69 × 10-3 molar
e) 5.38 molar
65. What mass of glucose, C6H12O6, is necessary to prepare 2.50 × 102 milliliters of a 1.00 molar aqueous
solution?
a) 7.20 × 102 g
b) 4.50 × 101 g
c) 2.50 × 10-1 g
d) 1.00 × 101 g
e) 2.50 × 101 g
66. What total volume of a 2.25 molar sodium chloride aqueous solution contains 4.5 × 10-1 moles of sodium
chloride formula units?
a) 1.0 mole
b) 2.3 mole
c) 2.0 × 10-1 mole
d) 2.0 × 10-2 mole
e) 4.5 × 10-2 mole
67. How many grams of sodium carbonate, Na2CO3, must be dissolved in 3.75 L of aqueous solution to yield a
molar concentration of 1.75 molar?
a) 2.02 × 10-2 g
b) 202 g
c) 2.92 × 10-1 g
d) 696 g
e) 6.96 g
68. What is the volume of a 1.28 molar aqueous sodium chloride, NaCl, solution that contains 32 grams of
sodium chloride?
a) 7.0 × 10-1 L
b) 7.0 × 102 L
c) 6.8 × 10-4 L
d) 1.2 × 104 L
e) 1.4 × 10-1 L
69. What is the final molar concentration of a sodium hydroxide (NaOH) solution if 25 milliliters of a 0.350
molar NaOH solution is diluted to 1.00 liter?
a) 7.1 × 10-2 molar
b) 14 molar
c) 1.4 molar
d) 8.75 molar
e) 8.75 × 10-3 molar
70. How many milliliters of a 0.100 molar sulfuric acid, H2SO4, solution is needed to make 25.0 milliliters of a
5.00 × 10-3 molar solution?
a) 1.25 mL
b) 800 mL
c) 8.00 mL
d) 125 mL
e) .125 mL
71. When the following chemical reaction is properly balanced the coefficients are:
C3H8 + O2  CO2 + H2O
a) 0, 5, 3, 4
b) 1, 5, 3, 4
c) 2, 11, 6, 8
d) 2, 12, 6, 16
e) 3, 13, 9, 12
72. Write the following word equation as a balanced chemical equation: Aluminum bromide reacts with
chlorine to yield aluminum chloride and bromine.
a) AlBr + Cl  AlCl + Br
b) 2AlBr + Cl2  2AlCl + Br2
c) AlBr2 + Cl2  AlCl2 + Br2
d) 2AlBr3 + 2Cl3  2AlCl3 + 6Br
d) 2AlBr3 + 3Cl2  2AlCl3 + 3 Br2
73. Write the following word equation as a balanced chemical equation: Copper reacts with sulfuric acid to
yield copper(II)sulfate, water, and sulfur dioxide.
a) Cu + 2 H2SO4  CuSO4 + 2 H2O + SO2
b) 2 Cu + 3 H2S  Cu2S + 3 H2O + S2O
c) Cu + H2SO4  Cu2SO4 + H2O + SO2
d) 2 Cu + 2 H2SO4  2 CuSO4 + 4 H2O + S2O
e) Cu + H2S + 3O2  CuSO4 + H2O + SO2
74. Write the following word equation as a balanced chemical equation: Hydrogen gas reacts with nitric oxide
to yield water and nitrogen gas.
a) 2 H + NO  H2O + N
b) H2 + NO  H2O + N
c) 2 H2 + 2NO  2 H2O + N2
d) 4 H + 2NO  2 H2O + N2
e) 4 H + 2NO  2 H2O + 2 N
75. When the following chemical equation is balanced, with all whole numbers, the coefficient for CO2 is:
C8H18 + O2  CO2 + H2O
a) 16
b) 12
c) 10
d) 9
e) 8
76. When the following chemical reaction is balanced, with all whole numbers, the coefficient for oxygen is:
S8 + O2  SO3
a) 1
b) 3
c) 4
d) 6
e) 12
77. When the following chemical reaction is balanced, with all whole numbers, the coefficients are:
FeCl3 + NaOH  Fe(OH)3 + NaCl
a) 1, 3, 1, 3
b) 3, 1, 3, 1
c) 3, 2, 3, 2
d) 2, 3, 2, 3
e) 3, 1, 1, 3
78. When the following chemical reaction is balanced, with all whole numbers, the coefficients are:
Ca(OH)2 + H3PO4  Ca3(PO4)2 + H2O
a) 1, 2, 1, 6
b) 3, 2, 1, 6
c) 2, 3, 2, 3
d) 3, 2, 4, 6
e) 3, 2, 3, 2
79. When the following chemical reaction is balanced, with all whole numbers, the coefficients are:
KClO3  KCl + O2
a) 1, 1, 2
b) 1, 1, 3
c) 2, 1, 3
d) 2, 2, 3
e) 2, 2, 2
80. When the following chemical reaction is balanced, with all whole numbers, the coefficients are:
CO2 + H2O  C6H12O6 + O2
a) 6, 6, 1, 6
b) 3, 3, 1, 3
c) 6, 3, 3, 6
d) 12, 3, 2, 6
e) 12, 3, 2, 12
81. Which of the following substances would be considered a weak electrolyte?
a) a strong acid
b) a soluble salt
c) a weak acid
d) a soluble base
e) an inert gas
82. Which of the following would NOT be classified as a strong acid?
a) HClO3
b) HI
c) HBr
d) HClO4
e) HClO2
83. When acetic acid, H3CCOOH, is dissolved in water, all of the following should be present in the solution,
EXCEPT:
a) H3CCOOH
b) H2O
c) H3O+
d) H3C+
e) H3CCOO84. What type of reaction is the following?
AgNO3(aq) + NH4Cl(aq)  NH4NO3(aq) + AgCl(s)
a) redox
b) single displacement
c) precipitation
d) decomposition
e) combustion
85. Which of the following state symbols is not properly defined?
a) (s), solid
b) (l), liquid
c) (g), gas
d) (aq), aqueous
e) They are all correct.
86. Write the correct balanced precipitation reaction when aqueous lead(II)chloride is mixed with aqueous
lithium sulfate to yield the precipitate lead(II)sulfate.
a) PbCl2(aq) + Li2SO4(aq)  PbSO4(s)
b) PbCl2(aq) + Li2SO4(aq)  PbSO4(s) + 2 LiCl(aq)
c) PbCl2(aq) + Li2SO4(aq)  PbSO4(s) + 2 LiCl(s)
d) PbCl2(aq) + Li2SO4(aq)  PbSO4(s) + LiCl(aq)
e) Pb2Cl2(aq) + Li2SO4(aq)  Pb2SO4(s) + 2 LiCl(s)
87. The total ionic equation for the following reaction is:
AgNO3(aq) + NaCl(aq)  NaNO3(aq) + AgCl(s)
+
a) Ag (aq) + NO3-(aq) + Na+(aq) + Cl-(aq)  Na+(aq) + NO3-(aq)
b) Ag+(aq) + NO3-(aq) + Na+(aq) + Cl-(aq)  Na+(aq) + NO3-(aq) + AgCl(s)
c) NO3-(aq) + Na+(aq)  Na+(aq) + NO3-(aq)
d) Ag+(aq) + Cl-(aq)  AgCl(s)
e) Ag+(s) + NO3-(aq) + Na+(aq) + Cl-(s)  Na+(aq) + NO3-(aq) + AgCl(s)
88. The total ionic equation for the following reaction is:
Fe2(SO4)3(aq) + 6NaOH(aq)  2Fe(OH)3(s) + 3Na2SO4(aq)
3+
a) 2Fe (aq) + 3SO42-(aq) + 6Na+(aq) + 6OH-(aq)  2Fe(OH)3(s) + 6Na+(aq)
+ 3SO42-(aq)
b) 2Fe3+(aq) + 3SO42-(aq) + 6Na+(aq) + 6OH-(aq)  6Na+(aq) + 3SO42-(aq)
c) 3SO42-(aq) + 6Na+(aq)  6Na+(aq) + 3SO42-(aq)
d) 2Fe3+(s) + 3SO42-(aq) + 6Na+(aq) + 6OH-(s)  2Fe(OH)3(s) + 6Na+(aq) + 3SO42-(aq)
e) 2Fe3+(aq) + 6OH-(aq)  2Fe(OH)3(s)
89. The net ionic equation for the following reaction:
AgNO3(aq) + NaCl(aq)  NaNO3(aq) + AgCl(s)
+
a) Ag (aq) + NO3-(aq) + Na+(aq) + Cl-(aq)  Na+(aq) + NO3-(aq)
b) Ag+(aq) + NO3-(aq) + Na+(aq) + Cl-(aq)  Na+(aq) + NO3-(aq) + AgCl(s)
c) NO3-(aq) + Na+(aq)  Na+(aq) + NO3-(aq)
d) Ag+(aq) + Cl- (aq)  AgCl(s)
e) Ag+(s) + NO3-(aq) + Na+(aq) + Cl-(s)  Na+(aq) + NO3-(aq) + AgCl(s)
90. The net ionic equation for the following reaction is:
HBr (aq) + KOH(aq)  KBr(aq) + H2O(l)
a) H+(aq) + Br-(aq) + K+(aq) + OH-(aq)  K+(aq) + Br-(aq) + H+(aq) + OH-(aq)
b) H+(aq) + Br-(aq) + K+(aq) + OH-(aq)  K+(aq) + Br-(aq) + H2O (l)
c) H+(aq) + Br-(aq) + K+(aq) + OH-(aq)  K+(aq) + Br-(aq) + H+(l) + OH-(l)
d) Br-(aq) + K+(aq)  K+(aq) + Br-(aq)
e) H+(aq) + OH-(aq)  H2O(l)
91. All of the following are strong bases, EXCEPT:
a) NaOH
b) KOH
c) Ca(OH)2
d) Mg(OH)2
e) Ba(OH)2
92. All of the following are strong bases, EXCEPT:
a) NaOH
b) KOH
c) Na2O
d) NH3
e) Ba(OH)2
93. Which of the following is a strong acid?
a) HF
b) CH3COOH
c) NH3
d) CH3NH2
e) HI
94. Of the following, the compound that is classified as a salt is:
a) HF
b) HI
c) NaI
d) Na2O
e) NaOH
95. When ammonia is combined with hydrochloric acid, the products are:
a) NH4Cl + H2O
b) NH4Cl + OH- + H2
c) NH3Cl + H2O
d) NH3Cl + H2
e) NH4Cl + OH96. When barium hydroxide is combined with sulfuric acid, the products are:
a) Ba(OH)2 + H2SO4
b) BaSO4 + H2O
c) BaSO4
d) H2O
e) BaSO4 + H3O+
97. Of the following, the compound that is classified as a salt is:
a) KI (correct)
b) KOH
c) H2O
d) HI
e) H3O+
98. The net ionic equation for the following chemical reaction is:
HF(aq) + KOH(aq)  KF(aq) + H2O(l)
a) HF(aq) + K+(aq) + OH-(aq)  K+(aq) + F-(aq) + H+(l) + OH-(l)
b) HF(aq) + K+(aq) +  K+(aq) + F-(aq) + H+(l)
c) HF(aq) + K+(aq) + OH-(aq)  K+(aq) + F-(aq) + H2O(l)
d) HF(aq) + OH-(aq)  F-(aq) + H2O(l)
e) HF(aq) + K+(aq)  K+(aq) + H2O(l)
99. The net ionic equation for the following chemical reaction is:
2 CH3COOH(aq) + Ba(OH)2(aq)  Ba(CH3COO)2(aq) + 2H2O(l)
a) 2CH3COO-(aq) + H+(aq) + Ba2+(aq) + 2OH-(aq)  Ba2+(aq) + 2CH3COO-(aq)
+ 2H2O(l)
b) 2H+(aq)+ + 2OH-(aq)  2H2O(l)
c) 2CH3COOH(aq) + 2OH-(aq)  2CH3COO-(aq) + 2H2O(l)
d) Ba2+(aq) + 2OH-(aq)  Ba2+(aq) + 2H2O(l)
e) 2CH3COO-(aq) + H+(aq) + 2OH-(aq)  2CH3COO-(aq) + 2H2O(l)
100. The total ionic equation for the following reaction is:
2CH3COOH(aq) + Ba(OH)2(aq)  Ba(CH3COO)2(aq) + 2H2O(l)
a) 2CH3COO-(aq) + H+(aq) + Ba2+(aq) + 2OH-(aq)  Ba2+(aq) + 2CH3COO-(aq) + 2H2O(l)
b) 2H+(aq)+ + 2OH-(aq)  2H2O(l)
c) 2CH3COOH(aq) + Ba2+(aq) + 2OH-(aq)  2CH3COO-(aq) + Ba2+(aq) + 2H2O(l)
d) Ba2+(aq) +2OH-(aq)  Ba2+(aq) + 2H2O(l)
e) 2CH3COO-(aq) + H+(aq) + 2OH-(aq)  2CH3COO-(aq) + 2H2O(l)
101. Determine the oxidation number on sulfur in SO42-.
a) +4
b) -4
c) +6
d) -6
e) -2
102. Determine the oxidation number on phosphorus in P2O5.
a) +1
b) -1
c) +5
d) -5
e) +10
103. Determine the oxidation number on chromium in Cr2O72-.
a) +2
b) +3
c) +4
d) +5
e) +6
104. Determine the oxidation number on nitrogen in NaNO3.
a) -2
b) -5
c) +2
d) +5 (correct)
e) +6
105. Considering the following reaction, what is undergoing reduction?
2Na + Cl2  2NaCl
a) insufficient information to determine
b) Na and Cl2
c) Na
d) Cl2
e) NaCl
106. Considering the following reaction, what is undergoing reduction?
2H2 + O2  2H2O
a) insufficient information
b) H2 and O2
c) H2
d) O2
e) H2O
107. Considering the following reaction, what is undergoing oxidation?
Fe + ZnCl2  FeCl2 + Zn
a) Fe and Cl2
b) Fe and Zn
c) Fe
d) Zn
e) Cl2
108. Considering the following reaction, what is undergoing oxidation?
Cl2 + 2NaBr  Br2 + 2NaCl
a) Na
b) Na and Br2
c) Brd) Cl2
e) Na+
109. Balance the following net ionic redox reaction:
Fe + Ag+  Fe2+ + Ag
a) Fe + Ag+  Fe2+ + Ag
b) 2Fe + Ag+  Fe2+ + 2Ag
c) Fe + 2Ag+  Fe2+ + 2Ag
d) 2Fe + Ag+  2Fe2+ + Ag
e) Fe + 2Ag+  Fe2+ + Ag
110. Balance the following net ionic redox reaction:
Ca + Sb3+  Ca2+ + Sb
a) Ca + Sb3+  Ca2+ + Sb
b) 2Ca + Sb3+  Ca2+ + 3Sb
c) Ca + 2Sb3+  3Ca2+ + Sb
d) 3Ca + 2Sb3+  3Ca2+ + 2Sb
e) 2Ca + 3Sb3+  2Ca2+ + 3Sb
111. How many moles of calcium carbonate are produced when 2 moles of calcium cyanide react with excess
water, according to the following balanced equation:
Ca(CN)2 + 3 H2O  CaCO3 + 2NH3
a) 1 mole
b) 2 moles
c) 3 moles
d) 4 moles
e) insufficient information
112. How many moles of hydrochloric acid are necessary to react completely with 4 moles of aluminum
according to the following chemical reaction?
2Al + 6HCl  2AlCl3 + 3H2
a) 1 mole
b) 2 moles
c) 4 moles
d) 8 moles
e) 12 moles
113. How many moles of hydrogen are necessary to completely react with 10 moles of carbon monoxide in the
following chemical reaction?
CO + 2H2  CH3OH
a) 1 mole
b) 2 moles
c) 5 moles
d) 10 moles
e) 20 moles
114. Given 4 moles of iron and 6 moles of chlorine, how many moles of iron(III)chloride can be formed
according to the following chemical reaction?
2Fe + 3Cl2  2FeCl3
a) 1 mole
b) 2 moles
c) 3 moles
d) 4 moles
e) 6 moles
115. Given 8 moles of methane and 12 moles of chlorine, how many moles of carbon tetrachloride will be
formed according to the following chemical reaction?
CH4 + 4Cl2  CCl4 + 4HCl
a) 1 mole
b) 2 moles
c) 3 moles
d) 8 moles
e) 12 moles
116. Given 8 moles of aluminum in the following chemical reaction, how many moles of copper(II)sulfate
must be supplied to react away all the aluminum?
2Al + 3 CuSO4  Al2(SO4)3 + 3 Cu
a) 2 moles
b) 3 moles
c) 6 moles
d) 8 moles
e) 12 moles
117. What mass of potassium chloride would be produced upon the decomposition of 15 grams of potassium
chlorate, according to the following balanced decomposition reaction?
2KClO3  2KCl + 3O2
a) 4.5 g
b) 9.1 g
c) 15 g
d) 18 g
e) 30 g
118. How many grams of oxygen must be supplied to completely burn 26 grams of acetylene according to the
following balanced combustion reaction?
2C2H2 + 5O2  4CO2 + 2H2O
a) 8.5 g
b) 32 g
c) 65 g
d) 80 g
e) 160 g
119. How many grams of carbon dioxide will be formed by the decomposition of 68 grams of calcium
carbonate according to the following balanced decomposition reaction?
CaCO3  CaO + CO2
a) 30 g
b) 60 g
c) 68 g
d) 130 g
e) 260 g
120. How many grams of water can be produced in the complete combustion (excess oxygen) of 216 grams of
octane according to the following balanced combustion reaction?
2 C8H18 + 25 O2  16 CO2 + 18 H2O
a) 0.222 g
b) 162 g
c) 254 g
d) 324 g
e) 1.17 × 102 g
121. How many grams of water can be produced when 12 grams of zinc oxide react with 12 grams of
hydrochloric acid according to the following balanced chemical equation?
ZnO + 2HCl  ZnCl2 + H2O
a) 2.7 g
b) 6.0 g
c) 12 g
d) 24 g
e) 36 g
122. How many grams of sodium chloride can be formed when 25 grams of iron(II)chloride react with 50
grams of sodium phosphate according to the following balance chemical equation?
3FeCl2 + 2Na3PO4  Fe3(PO4)2 + 6NaCl
a) 13 g
b) 23 g
c) 33 g
d) 50 g
e) 75 g
123. How many grams of water are produced when 45 grams of benzene burn in 15 grams of oxygen according
to the following balanced chemical equation?
2C6H6 + 15O2  12CO2 + 6H2O
a) 0.19 g
b) 1.7 g
c) 3.4 g
d) 31 g
e) 50 g
124. How many grams of nitric oxide are produced when 26 grams of ammonia burn in 26 grams of oxygen
according to the following balanced chemical equation?
4NH3 + 5O2  4NO + 6H2O
a) 13 g
b) 20 g
c) 26 g
d) 46 g
e) 52 g
125. When 26 grams of ammonia burn in 26 grams of oxygen, according to the following balanced equation,
what is the limiting reagent?
4NH3 + 5O2  4NO + 6H2O
a) NH3
b) O2
c) NO
d) H2O
e) NH3 and O2
126. When 12 grams of zinc oxide react with 12 grams of hydrochloric acid according to the following
balanced chemical equation, what is the limiting reagent?
ZnO + 2HCl  ZnCl2 + H2O
a) ZnO
b) HCl
c) ZnCl2
d) H2O
e) ZnO and HCl
127. How many milliliters of a 0.50 molar solution of calcium hydroxide are necessary to completely neutralize
40 milliliters of a 0.25 molar nitric acid solution according to the following balanced neutralization reaction?
2HNO3(aq) + Ca(OH)2(aq)  Ca(NO3)2(aq) + H2O(l)
a) 40 mL
b) 20 mL
c) 10 mL
d) 5 mL
e) 1 mL
128. How many milliliters of a 0.40 molar solution of hydrochloric acid is necessary to neutralize 25 milliliters
of a 0.20 molar sodium hydroxide solution?
a) 50 mL
b) 25 mL
c) 20 mL
d) 12.5 mL
e) 10.5 mL
129. How many milliliters of a 0.70 molar solution of barium hydroxide, Ba(OH)2, is necessary to neutralize 55
milliliters of a 1.4 molar solution of sulfuric acid, H2SO4?
a) 220 mL
b) 110 mL
c) 55 mL
d) 22 mL
e) 11 mL
130. For a particular chemical reaction the theoretical yield was 12 grams of product, but the actual yield was 3
grams. What is the percent yield of this reaction?
a) 100%
b) 75%
c) 50%
d) 25%
e) insufficient information
131. For a particular chemical reaction the theoretical yield was 3 grams of product, but the actual yield was 12
grams. What is the percent yield of this reaction?
a) 100%
b) 75%
c) 50%
d) 25%
e) Impossible occurrence
1. d) 5.7 × 102
2. e) 81
3. c) 10863
4. d) 1, 3, 4, 5, 3, 6
5. d) 5 × 103 mm
6. c) 1.42 × 104 g
7. e) 1.3 g · cm-3
8. c) 190 mL · min-1
9. b) about 1 year
10 a) 110 g
11. a) lb · ft-3
12.b) 31.0 mL
13 d) 1 430 mm2
14e) 43 m · s-1
15. e) a compound
16. a) a heterogeneous mixture
17. a) gamma rays
18. c) All atoms are composed of
electrons, protons, and neutrons.
19. c) The nuclear model in
which the positive charge is held
densely in the center of the atom is
no longer accepted, because it was
proposed over 100 years ago.
20. c) 10 protons, 10 electrons, 11
neutrons
21. c) 6 protons, 6 electrons, 6
neutrons
22. a) fluorine
23. c) barium
24. d) fluorine
25. a) bromine
26. e) Na, Si, B, Ca, S
27. e) KCl
28. d) BrCl
29. c) S2+
30. c) CaF2
31. b) potassium sulfide, KS
32. b) BrCl5
33. d) ammonium nitrite
34. b) sulfur trioxide
35. c) sodium oxide
36. d) potassium perchlorate
37. a) CH4, carbon tetrahydride
38. d) tin, Ti
39. b) mercury, M
40. c) C2H2, dicarbon dihyrdide
41. d) They both have the same
number of molecules.
42. c) 9 moles
43. e) 5.4199 × 1024 atoms
44. d) 2.5 moles
45. a) 4 moles
46 a) 187.57 g·mol-1
47. c) 68.14 g·mol-1
48. e) 180.16 g·mol-1
49. b) 2.84 moles
50. a) 1.71 × 1024 molecules
51. c) 1.1 × 103 g
52. d) 7.11 × 1024 formula units
53. a) 88.81%
54 d) 64% N, 36% O
55. a) 27.05% Na, 16.48% N,
56.47% O
56. c) C3H3O
57. c) SOCl2
58. d) N2O
59. c) C6H6
60. e) C3H2Cl
61. c) Within a solution, the
component in the least amount is
called the solvent.
62. d) combustion train
63. c) 4.00 molar
64. a) 2.69 molar
65. b) 4.50 × 101 g
66 c) 2.0 × 10-1 mole
67. d) 696 g
68. a) 7.0 × 10-1 L
69. e) 8.75 × 10-3 molar
70. a) 1.25 mL
71. b) 1, 5, 3, 4
72. d) 2AlBr3 + 3Cl2 2AlCl3 + 3
Br2
73. a)Cu +2H2SO4
CuSO4+2H2O+SO2
74. c) 2 H2 + 2NO  2 H2O +
N2
75.
76.
77.
78.
79
80.
81.
82.
83.
84.
85.
a) 16
e) 12
a) 1, 3, 1, 3
b) 3, 2, 1, 6
d) 2, 2, 3
a) 6, 6, 1, 6
c) a weak acid
e) HClO2
d) H3C+
c) precipitation
e) They are all correct.
86. b) PbCl2(aq) + Li2SO4(aq) 
PbSO4(s) + 2 LiCl(aq)
87. b) Ag+(aq) + NO3-(aq) + Na+(aq)
+ Cl-(aq)  Na+(aq) + NO3-(aq) +
AgCl(s)
88. a) 2Fe3+(aq) + 3SO42-(aq) +
6Na+(aq) + 6OH-(aq)  2Fe(OH)3(s)
+ 6Na+(aq)
+ 3SO42-(aq)
89. d) Ag+(aq) + Cl- (aq) 
AgCl(s)
90. e) H+(aq) + OH-(aq)  H2O(l)
91.
92.
93
94.
95.
96.
97.
d)
d)
e)
c)
a)
b)
a)
Mg(OH)2
NH3
HI
NaI
NH4Cl + H2O
BaSO4 + H2O
KI
98. d) HF(aq) + OH-(aq)  F(aq) + H2O(l)
99. c) 2CH3COOH(aq) + 2OH-(aq)
 2CH3COO-(aq) + 2H2O(l)
100. c) 2CH3COOH(aq) + Ba2+(aq)
+ 2OH-(aq)  2CH3COO-(aq) +
Ba2+(aq) + 2H2O(l)
101. c) +6
102. c) +5
103. e) +6
104. d) +5
105. d) Cl2
106. d) O2
107. c) Fe
108. c) Br109. c) Fe + 2Ag+  Fe2+ + 2Ag
110. d) 3Ca + 2Sb3+  3Ca2+ + 2Sb
111. b) 2 moles
112. e) 12 moles
113. e) 20 moles
114. d) 4 moles
115. c) 3 moles
116. e) 12 moles
117. b) 9.1 g
118. d) 80 g
119. a) 30 g
120. d) 324 g
121. a) 2.7 g
122. b) 23 g
123. c) 3.4 g
124. b) 20 g
125. b) O2
126. a) ZnO
127. c) 10 mL
128. d) 12.5 mL
129b) 110 mL
130 d) 25%
131. e) impossible occurrence